**Contents**show

## How many coulomb’s of electricity are required for the reduction of 1 equivalent mno4 in acidic medium?

Therefore, 5 mol of electrons are required to reduce 1 mol of MnO-4 ions).

## How many coulombs of electricity are required for reduction of 1 mole of mno4?

93×105C.

## How many coulombs are required for the reduction of IMOL of mno4 to Mn 2?

28×105C.

## How many coulombs of electricity are required for reduction of 1 mole of cr2o7?

1×96500 C.

## How many coulombs are required for complete oxidation of 90 g of h2o?

1. 93×104C.

## How many coulombs of electricity are required for the oxidation of 1 mole of h2o?

The electric charge required to oxidise 1 mole of [{{text{H}}_{text{2}}}{text{O}}] to [{text{O}}]is 193000 Coulomb. Thus, the correct option is (B).

## How many coulombs of electricity are required for the reduction of one mole of MnO4 negative to Mn to positive?

Because in MnO4- the oxidation number of Mn is +7 and in Mn2+ the oxidation number of Mn is +2. Faraday’s constant is 96500 C/mol. Simply multiply 96500 by 5 then by 0.05, which gives 24125 C.

## How many Faraday of electricity is required to reduce 1 mole of MnO4 minus ions to Mn 2 ions?

How many faradays are required to reduce one moleof MnO_(4)^(-) to Mn^(2+)? Number of faradays is equal to the change in oxidation state. Since oxidation state of Mn decreases by 5 units (from +7 to +2), five faradays is needed.

## How many moles of electrons are required for the reduction of 1 mole of MnO4?

Hence 5 moles of electrons are required for 1 mole of MnO−4 .

## How many coulombs are in an electric charge?

One coulomb is equal to the amount of charge from a current of one ampere flowing for one second. One coulomb is equal to the charge on 6.241 x 10^{18} protons. The charge on 1 proton is 1.6 x 10^{–}^{19} C. Conversely, the charge of an electron is -1.6 x 10^{–}^{19} C.

## How many Coulomb of electricity are consumed when 100 ma current is passed through a solution of agno3 for half an hour during electrolysis?

8g/cm3]

## How many coulombs of electricity are required for Al to Al3+?

1 mole of electrons carry a charge of 1.6E-19 *6.022E23 coulomb, which equals 96500 C and is called 1 Faraday. For 1 mole of Al3+, we need 3 moles of electrons and that is equal to 3 Faraday of charge i.e. 3*96500 C.

## What amount of electric charge is required for the reduction of 1 mole of cr2o7 2 to cr3 +?

9650C.

## How many moles are in a PT?

1 grams Pt is equal to 0.0051261546663386 mole.

## When 9650 coulombs of electricity is passed through a solution of copper sulphate the amount of copper deposited is?

25mol.